Ionic EquilibriumHard
Question
The silver ion concentration in a 0.2 M solution of Ag(NH3)2NO3 is (Kdiss = 6.8 × 10−8, 1.53 = 3.4)
Options
A.0.2 M
B.1.5 × 10−3 M
C.1.16 × 10−4 M
D.6.8 × 10−8 M
Solution
$Ag\left( NH_{3} \right)_{2}^{+} \rightleftharpoons Ag^{+} + 2NH_{3}$;Keq = 6.8 × 10–8
0.2 M 0 0
Eqn 0.2 – x = 0.2 M xM 2xM
Now, $6.8 \times 10^{- 8} = \frac{x \times (2x)^{2}}{0.2}$
$\Rightarrow x = 1.5 \times 10^{- 3}\text{ M = }\left\lbrack Ag^{+} \right\rbrack$
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
In 500 ml of 2.5 × 10−5 M – AgNO3 solution, 2000 ml of 5.0 × 10−2 M – NaCl solution is added. The mass of precipitate of...Sodium nitroprusside when added to an alkaline solution of sulphide ions produce a :-...Heat of neutralisation of oxalic acid is -25.4 K cal mol-1 using strong base NaOH. Hence enthalpy change of the process ...The solubility of PbCl2 when it is 80% ionized is...The precipitate of CaF2 (Ksp = 1.7 × 10-10) is obtained, when equal volumes of the following are mixed :...